Collision Theory plays a vital role in this fast-developing world and results in chemical reactions.
Collision theory in chemistry allows scientists to predict a rate constant of a chemical reaction which can be used to determine reaction rates. This theory was developed by Max Trautz and William Lewis to derive meaningful insights into these chemical reactions.
Collision theory states that the rate of a chemical reaction is directly proportional to the number of collisions occurring between the reactant molecules. In simple terms, the collision theory in chemistry explains what initiates chemical reactions. Theoretically, the more that the reactant molecules collide with one another, the faster the rate of reaction becomes. In reality, however, only a small fraction of the collisions are what we term effective collisions, which are the only type of collision that results in the creation of a product.
To initiate effective collisions, reactant molecules are required to have activation energy, which is the minimum amount of energy required to undergo a reaction. The count of molecules possessing sufficient energy is all dependent on the reactant's temperature. If these reactants do not possess their required activation energy, they bounce back from each other without even reacting.
Collision theory is based on three postulates: The rate of reaction is proportional to the rate of reactant collision molecules. The reacting element should collide to allow contact between the atoms, which are meant to be bonded together. There must be sufficient energy to allow mutual penetration of the reactants so that the electrons can again arrange and form new bonds.
1. What is collision theory?
Collision theory defines that the chemical reaction rate is proportional to the number of collisions occurring between the reactant molecules. This occurs at certain chemical reactions and rates.
2. What are the 4 points of collision theory?
3. What are the three postulates of collision theory?
4. What equation is used for collision theory?
K ∝ e-Ea/RT
K = A e-Ea/RT
where, A is the frequency factor, Ea is the activation energy, R is gas constant and T is the absolute temperature
This is the Arrhenius equation, and the collision theory equation is accommodated in this only.
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